![Representing Electron ConfigurationsOrbital NotationNa__ __ __ __ __ __ 1s 2s 2p 3sElectron-Configuration NotationNa 1s22s22p63s1Noble-Gas NotationNa [Ne] 3s1Write the electron configuration, orbital notation, and noble gas notation for an atom whose atomic number is:20817Writing Electron Configuration](https://image.slidesharecdn.com/chapter3-3applied-100331135620-phpapp01/85/Applied-Chapter-3-3-Electron-Configuration-16-320.jpg)
Applied Chapter 3.3 : Electron Configuration
- 2. Objective 1:Compare the Rutherford, Bohr, and Quantum models of the atom.Rutherford’s model of atomElectrons orbit the nucleus just as planets orbit the sunBohr’s model of the atomElectrons travel around the nucleus in specific energy level Quantum – difference in energy between two energy levels. Bohr Video
- 3. Quantum model of the atomElectrons are found in orbitals around the nucleus of atom.Orbital (electron cloud) – region of atom where there is a high probability of finding electrons
- 4. Electrons – Act like particles and wavesParticles Cathode ray tubePhotoelectric effectWavesElectromagnetic spectrumLine-emission spectrum
- 5. Objective 2:Explain how the wavelengths of light emitted by an atom provide information about energy levels.Light provides information about electronsNeonElectrons start in ground stateLowest possible energy levelRun electricity through gasElectrons absorb this energyThey move to excited stateElectron has more energy than normalQuickly fall back to ground stateEnergy is emitted as lightLight has a specific wavelengthDetermines color (and line-emission spectrum)KryptonArgon
- 7. Objective 3:List the four quantum numbers, and describe their significance.Quantum numbers:Number that specifies the properties of electronsTells where they are in the atom.Principle quantum number ( n )Main energy leveln = 1,2,3,4,5 …….. InfinityDistance from nucleusAngular Momentum quantum number ( l )indicates the shape of the orbitall = 0, 1, 2, 3 s p d fspd
- 8. Magnetic (m) orientation of orbital around nucleusm =-1,0,+1m = 0m =-2,-1,0,+1,+2
- 9. 4. Spin Quantum Number ( +1/2, -1/2) or , Indicates the two fundamental spin states of electron in an orbitalSingle orbital can hold a maximum of 2 electrons
- 11. Quantum Numbers of the 1st thirty atomic orbitalsTotal Electrons in n281832
- 12. Objective 4Write the electron Configuration of an atom by using the Pauli Exclusion principle and the aufbau principle.Electron ConfigurationThe arrangement of electrons in an atomLowest-energy arrangement – ground-state electron configurationRules Governing Electron ConfigurationAufbau Principle – electron occupies the lowest-energy orbital that can receive it. Pg. 105Pauli exclusion Principle – no two electrons in the same atom can have the same set of four quantum numbersHund’s Rule – orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin.
- 13. Aufbau principle 4f 5f 6f 7f 3d 4d 5d 6d 7d 2p 3p 4p 5p 6p 7p1s 2s 3s 4s 5s 6s 7s** Gives the order of energy levels and orbitals
- 15. Hund’s Rule
- 16. Representing Electron ConfigurationsOrbital NotationNa__ __ __ __ __ __ 1s 2s 2p 3sElectron-Configuration NotationNa 1s22s22p63s1Noble-Gas NotationNa [Ne] 3s1Write the electron configuration, orbital notation, and noble gas notation for an atom whose atomic number is:20817Writing Electron Configuration